Chemistry Practi ce -1 st Semester Safety and Measurement

Lab Safety1. Flammable materials, like alcohol, should never be dispensed or used near

a. an open door.b. an open flame.c. another student.d. a sink.

2. If a laboratory fire erupts, immediatelya. notify your instructor.b. run for the fire extinguisher.c. throw water on the fire.d. open the windows.

3. Approved eye protection devices (such as goggles) are worn in the laboratorya. to avoid eye strain.b. to improve your vision.c. only if you don’t have corrective glasses.d. any time chemicals, heat or glassware are used.

4. If you wear contact lenses in the school laboratory,a. take them out before starting the lab.b. you do not have to wear protective goggles.c. advise your science instructor that you wear contact lenses.d. keep the information to yourself.

5. If you do not understand a direction or part of a lab procedure, you shoulda. figure it out as you do the lab.b. try several methods until something works.c. ask the instructor before proceeding.d. skip it and go on to the next part.

6. After completing an experiment, all chemical wastes should bea. left at your lab station for the next class.b. disposed of according to your instructor’s directions.c. dumped in the sink.d. taken home.

7. If a lab experiment is not completed, you shoulda. discuss the issue with your instructor.b. sneak in after school and work alone.c. come in during lunch and finish while eating lunch.d. make up some results.

8. You are heating a substance in a test tube. Always point the open end of the tubea. toward yourself.b. toward your lab partner.c. toward another classmate.

d. away from all people.

9. You are heating a piece of glass and now want to pick it up. You shoulda. use a rag or paper towels.b. pick up the end that looks cooler.c. use tongs.d. pour cold water on it.

10. You have been injured in the laboratory (cut, burn, etc.). First you shoulda. visit the school nurse after class.b. see a doctor after school.c. tell the science instructor at once.d. apply first aid yourself.

11. When gathering glassware and equipment for an experiment, you shoulda. read all directions carefully to know what equipment is necessary.b. examine all glassware to check for chips or cracks.c. clean any glassware that appears dirty.d. All of the above.

12. You want to place a piece of glass tubing into a rubber stopper after the tubing has been fire polished and cooled. This is best done by

a. lubricating the tubing with water or glycerin.b. using a towel or cotton gloves for protection.c. twisting the tubing and stopper carefully.d. all of the above.

13. Personal eyeglasses provide as much protection asa. a face shield.b. safety glasses.c. splashproof chemical goggles.d. none of the above.

14. Long hair in the laboratory must bea. cut short.b. held away from the experiment with one hand.c. always neatly groomed.d. tied back or kept entirely out of the way with a hair band, hairpins, or other confining device.

15. In a laboratory, the following should not be worn.a. loose clothing.b. dangling jewelry.c. sandals.d. all of the above.

16. The following footwear is best in the laboratory.a. sandalsb. open-toed shoesc. closed-toed shoesd. shoes appropriate for the weather

17. Horseplay or practical jokes in the laboratory are

a. always against the rules.b. okay.c. not dangerous.d. okay if you are working alone.

18. If a piece of equipment is not working properly, stop, turn it off, and tella. the custodian.b. your lab partner.c. your best friend in the class.d. the science instructor.

19. If an acid is splashed on your skin, wash at once witha. soap.b. oil.c. weak base.d. plenty of water.

20. When you finish working with chemicals, biological specimens, and other lab substances, alwaysa. treat your hands with skin lotion.b. wash your hands thoroughly with soap and water.c. wipe your hands on a towel.d. wipe your hands on your clothes.

Precision and accuracy1. A measurement that closely agrees with accepted values is said to be _______.

a. Accurateb. Precisec. Reliabled. Significant

2. A measurement is said to have good precision if it _______.a. agrees closely with an accepted standard.b. agrees closely with other measurements of the same quantity.c. has a small number of significant figures.d. has a large number of significant figures.

3. The accuracy of a measurement:a. Is how close it is to the true valueb. Does not depend on the instrument being used to measure the objectc. Indicates that the measurement is also precised. Is something that scientists rarely achieve

4. A physicist who frequently carries out the same complex experiment is likely to have high ______.a. Accuracyb. Precisionc. Significanced. Scientific notation

5. Three groups of students measure the mass of a product from the same chemical reaction. The groups recorded data of 8.83 g, 8.84 g and 8.82 g. The known mass of the product from that reaction is 10.60g. The group values are ______.

a. Accurate but not Precise

b. Precise but not Accuratec. Accurate and precised. Neither accurate nor precise

6. Which experiment is least precise?a. Experiment Ib. Experiment IIc. Experiment IIId. Experiment IV

7. Which experiment is accurate?a. Experiment Ib. Experiment IIc. Experiment IIId. Experiment IV

8. Which experiment is accurate and precise?a. Experiment Ib. Experiment IIc. Experiment IIId. Experiment IV

9. Which experiment is precise but not accurate?a. Experiment Ib. Experiment IIc. Experiment IIId. Experiment IV

SI units1. What is the abbreviation for meter?

a. mb. Mc. Med. Mt

2. What is the abbreviation for liter?a. lb. Lc. Lid. Lt

3. What is the abbreviation for gram?a. gb. Gc. Grd. Gm

4. What is the abbreviation for decimeter?a. dmb. dcmc. damd. dem

5. What is the abbreviation for decameter?a. dmb. dcmc. damd. dem

6. What is the abbreviation for centigram?a. ctgb. cgc. cd. ceg

7. What is the abbreviation for kiloliter?a. kLb. Kc. kld. kil

8. What is the abbreviation for hectoliter?a. hecLb. heLc. hLd. H

9. What is the abbreviation for centigram?a. ctgb. cgc. cd. ceg

10. What is the abbreviation for milligram?a. MiGb. mgc. mmd. mLg

Significant figures1. How many significant digits are in the following number: _______?

a. 2b. 4c. 6d. 8

2. When you calculate the speed (in meters per second) in an experiment, your calculator display reads 12.666667. If you are asked to record your result to three significant figures, you should write:

a. 12.6 m/s.b. 12.7 m/s.c. 12.666 m/s.d. 12.667 m/s.

Express numbers in scientific notation when appropriate

1. Which of the following numbers would be the best choice to be written in scientific notation?a. 84b. 690c. 0.06d. 657000

2. Which of the following numbers would be the best choice to be written in scientific notation?a. 48b. 0.000987c. 0.04d. 934

3. What is the 0.00979g in scientific notation?a. 9.79 x 106gb. 9.79 x 10-5gc. 9.79 x 10-3gd. 979 x 10-5g

4. What is the 0.00000032mm in scientific notation?a. 3.2 x 10-7mmb. 3.2 x 107mmc. 32 x 10-7mmd. 32 x 107mm

5. What is the 700000000daL in scientific notation?a. 7 x 105daLb. 7 x 106daLc. 7 x 107daLd. 7 x 108daL

6. What is the 1870000km in scientific notation?a. 1.87 x 104kmb. 1.87 x 105kmc. 1.87 x 106kmd. 1.87 x 107km

7. What is the 5.3 x 10-2 in conventional notation?a. 0.53b. 0.053c. 53d. 530

8. Express 6.487 x 104 as a number.a. 6487b. 0.06487c. 64870d. 0.0006487

9. Express 3.2 x 10-3 as a number.a. 320b. 32000c. 0.032

d. 0.0032

Solve for unknown quantities by manipulating variables1. Which of the following liquids has the greatest density?

a. 13cm3 with a mass of 23 gb. 3.5 cm3 with a mass of 10gc. 0.022 cm3 with a mass of 0.10 gd. 54 cm3 with a mass of 45 g

2. Given 90 ml of hydrogen gas collected where the temperature is 27°C. How many ml will the Hydrogen occupy at 42°C? Pressure remains constant.

a. 12.6 mlb. 57.9 mlc. 140 mld. 412 ml

3. A gas sample occupies 300.o ml at 760 mmHg. What volume does the gas occupy at 400 mmHg?a. 157.9 mlb. 570 mlc. 1013 mld. 912,000 ml

4. A mass of air occupies a volume of 5.70 liters at a pressure of 0.520 atm. What is the new pressure if the same mass of air at the same temperature is transferred to a 2.00 Liter container?

a. 1.48 atmb. 2.96 atmc. 5.92 atmd. 7.88 atm

Use graphical, mathematical, and/or statistical models to express patterns and relationships inferred from sets of scientific data

1. Tom wanted to know how much fertilizer he should give his tomato plants. He gave different amounts of fertilizer to his plants. He then counted the number of tomatoes grown on each plant. His results are in the data table to the right. Which set of axes below is the BEST to use for graphing his results?

Amount of Fertilizer

Number of Tomatoes Produced

0 3100 4150 6250 8450 8

2. At 50 Pascals of pressure, how many ml of volume would be used?

a. 30 b. 40c. 35 d. 45

3. At 18 ml of volume, how many Pascals of pressure would

be used?a. 100 b. 80c. 70d. 75

Explain density qualitatively and solve density problems by applying an understanding of the concept of density.1. If you measured the density for a block of wood and then cut the wood in half and measured the density

of one of the halves, would you get different values for density? Why or why not?a. Yes, because by cutting the block of wood you essentially cut the amount of atoms in half

therefore lowering the density.b. Yes, because by cutting the block of wood you lowered the volume but not the mass.c. No, because the mass and volume are unchanged and therefore the density is unchanged as well

for each half of wood.d. No, because the mass and volume are both changed and the ratios stay the same and therefore the

density is unchanged for each half of wood.

2. Why is a sponge with a volume 20cm3 less dense then a brick with the same volume? a. The brick has more electrons than the sponge.b. Gravity exerts a greater force on the brick than the sponge.c. The sponge has less atoms packed closely together than the brick.d. None of the above.

3. The density of a material depends on ______.a. Its mass onlyb. Its volume onlyc. Its mass and volumed. Its weight

4. If a graduated cylinder had 50 milliliters of water and then a metal bolt were placed in the cylinder causing the water level to rise to 67 milliliters, what would be the volume of the bolt?

a. 67 mlb. 67 cm3

c. 17 mld. 50 ml

5. Suppose you were given two (2) balls of clay of equal size, shape and weight. One of the balls is flattened into a "pancake-shaped" piece. Which of the following statements is correct?

a. the pancake-shaped piece has greater density than the ballb. the two (2) pieces have the same densityc. there isn't enough information to determine which density is greater d. the ball of clay has greater density than the pancake-shaped piece

6. The test tube pictured below contains five (5) different substances. The substances were poured into the test tube and have positioned themselves from top to bottom based on their densities. The densities (g/cm3) of the five substances are as follows: Alcohol: 0.92, Gasoline: 0.7, Glycerin: 1.26, Mercury: 13.5, Water: 1.0. Choose the correct order of substances as they are in the test tube from top to bottom.

a. mercury, glycerin, water, alcohol, gasolineb. alcohol, water, gasoline, glycerin, mercury c. water, gasoline, glycerin, alcohol, mercuryd. gasoline, alcohol, water, glycerin, mercury

7. If you are given something with a volume of 150cm3, what is its volume in mL?a. 50 mLb. 150 gc. 450 mLd. 150 mL

8. If you are given the following data for a block of wood: length 3.5cm, width 4.7cm, height 9.0cm. What is the volume for the block of wood?

a. 148.05 cm3

b. 17.2 cm3

c. 0.083 cm3

d. 0.911 cm3

9. The density of iron (Fe) is 7.86g/cm3. You are given an unknown metal that has a mass of 224.6g. What would the volume of the sample be if it were iron?

a. 28.57 cm3

b. 28.57 gc. 28.57 g/cm3

d. 28.57 m

10. What mass of sucrose (density = 8g/mL) is needed to have a volume of 2mL?a. 4 gb. 0.25 gc. 8 gd. 16 g

11. Calculate the density of an unknown metal using the following information:-Mass of empty graduated cylinder 10.00 g-Volume of water before the addition of the metal 11.00 mL-Mass of graduated cylinder with 11.0 mL water 30.00 g-Volume reading after dropping metal in water 15.00 mL-Mass of graduated cylinder with water and metal 110.00 g

a. 20 g/mLb. 25 g/mLc. 320 g/mLd. 7.33 g/mL

12. What is the density of 20 g of oak that has a volume of 10 cm3?a. 200 g/cm3

b. 0.5 g/cm3

c. 200 gd. 2 g/cm3

13. If you have a sample of Uranium (density = 9.70 g/cm3) and a sample of iron (density = 7.87 g/cm3) and the samples have equal masses, then the following guess can be made about the relative volumes of these two samples.

a. The volumes of the metal samples cannot be compared due to lack of informationb. The volume of the Uranium sample is greater than the volume of the Iron samplec. The volume of the Iron sample is greater than the volume of the Uranium sampled. The volumes of the metal samples are equal

14. Suppose you took a piece of wood (density of 0.9 g/cm3) shown below, and cut it into 3 equal pieces. What would the density be of each piece?

a. 0.9 g/cm3 b. 0.3 g/cm3

c. 2.7 g/cm3

d. not enough information to find the answer

Scientific MethodIdentify and clarify research questions and design experiments

1. A hypothesis isa. the long side of a right triangle.b. an testable explanation that has yet to be proven by experiment.c. close agreement by competent observers of observations of the same phenomena.d. a synthesis of a large collection of information that includes guesses.

2. One difference between a hypothesis and a theory is that a hypothesisa. is a guess that has not been well tested, whereas a theory is a synthesis of well-tested guesses.b. is testable, whereas a theory is not testable.c. can be revised, whereas a theory cannot be revised.d. is not testable, whereas a theory is testable.

3. To test a scientific hypothesis you woulda. use the results of only the experiments that confirm the hypothesis.b. set up an experiment and look at the results.c. find the best result and report only that result.d. set up an experiment, look at the results, and repeat the experiment multiple times.

4. The scientific method is a:a. specialized lab write-upb. lab write-upc. method of observationd. method of problem solving

5. The 5 steps to the scientific method, in order, are:a. hypothesis, results, experiment, conclusion, questionb. hypothesis, question, results, experiment, conclusionc. question, hypothesis, experiment, results, conclusiond. question, hypothesis, experiment, conclusion, results

Design experiments so that variables are controlled and appropriate numbers of trials are used

1. A group of students uses clay to make boats of different shapes. All the boats they make have the same weight. The students add four tablespoons of salt in the water in a tank and mix the water. They place the boats in the tank and see if the boats float or sink. What can the students find out from doing just this experiment?

a. If shape affects whether the boats float or sink.

b. If weight affects whether the boats float or sink. c. If weight and the amount of salt in the water affect whether the boats float or sink. d. If shape, weight, and the amount of salt in the water affect whether the boats float or sink.

2. A science class wants to find out if the shape and the mass of objects made of the same metal affect how fast these objects sink in water. One group tests the effect of the shape, and another group tests the effect of the mass. The students who test the effect of the shape use three objects that have the same mass but different shapes. The students drop each object into a large water tank and measure how long it takes for each object to reach the bottom of the tank. Why is it important that the students use objects of the same mass?

a. By using objects of the same mass, the students can learn about both the effect of the mass and the effect of the shape.

b. By using objects of the same mass, the students can learn about the effect of the mass. c. If they do not use objects of the same mass, the students cannot learn about the effect of the

shape. d. It is NOT important for all the objects to have the same mass because the students are not testing

the effect of the mass.

3. A student thinks that there are three variables (X, Y and Z) that may affect the result of her experiment. What should the student do to find the effect of variable X on the result of the experiment?

a. Change variable X and keep variables Y and Z the same. b. Change variables Y and Z at the same time and keep variable X the same. c. Change variable X and Y at the same time and keep variable Z the same. d. Change variables X, Y, and Z at the same time.

4. A student thinks that there are two variables (X and Y) that may affect the result of her experiment. She decides to change only variable X and let variable Y stay the same. What can the student find out about the effects of variables X and Y?

a. If variable X affects the result of her experiment. b. If variable Y affects the result of her experiment. c. If both variables X and Y affect the result of her experiment. d. She cannot find out if either variable X or variable Y affects the result of her experiment.

5. A student conducted an experiment to _________________________________________. Using ___________________________________________________________. The student conducted one trial for each ___________________ and reported the results to the class. How is this likely to create an error in the study?

a. A limited number of trials causes mistakes to go unnoticedb. A limited number of trials leads to more accurate measurementsc. A limited number of trials means that the independent variable is not controlledd. A limited number of trials introduces bias into the investigation

6. Cory hypothesized that because copper conducts heat better than glass, water will boil faster in a copper pot than in a glass pot. In order to test this hypothesis, which of the following should be the dependent variable?

a. the type of pot used to boil the water b. the amount of water in each pot c. the time it takes the water to boil d. the temperature at which water boils

Explain the criteria that explanations must meet to be considered scientific (e.g., be consistent with experimental/observational evidence about nature, be open to critique and modification, use ethical reporting methods and procedures)

1. Which of the following is a reason to express scientific findings mathematically?a. The findings become more difficult to prove by experiment.b. The findings become easier to verify by experiment.c. The findings become more confusing.d. The findings become less appealing to the public.

MatterCompare the definition of matter and energy and the laws of conservation of mass and energy

1. Which statement about matter is TRUE? a. Atoms are not matter but they are contained in matter. b. Matter exists only when you can see it. c. Living things are not matter. d. Matter is made up of atoms.

2. Is air matter? Why or why not? a. Yes, because air is not alive. b. Yes, because air is made up of atoms. c. No, because air cannot be seen. d. No, because air does not take up space.

1. The windows of your school are made of glass. Which of the following statements describes the motion of the molecules that make up the glass?

a. The molecules of the glass are never moving. b. The molecules of the glass are always moving. c. The molecules of the glass move only when the sun warms the window. d. The molecules of the glass move only when the window is being opened or closed.

1. In a cup of liquid water, when would the water molecules stop moving? a. The molecules would stop moving if the liquid water in the cup became a solid. b. The molecules would stop moving if the liquid water in the cup became a gas. c. The molecules would stop moving if the liquid water in the cup became still. d. The molecules would not stop moving in the cup of liquid water.

2. Why can gases be compressed more easily than solids? a. Because the molecules of gases are softer than the molecules of solids b. Because the molecules of gases weigh less than the molecules of solidsc. Because the molecules of gases move faster than the molecules of solids d. Because the molecules of gases are farther apart than the molecules of solids

3. What happens when a cup of cold water warms up to room temperature? a. The size of the water molecules decreases. b. The number of water molecules increases. c. The mass of the water molecules decreases. d. The distance between the water molecules increases.

4. Why does liquid candle wax flow but solid candle wax does not? a. Because the molecules of liquid candle wax are softer than the molecules of solid candle wax b. Because the molecules of liquid candle wax weigh less than the molecules of solid candle wax c. Because the molecules of liquid candle wax are moving but the molecules of solid candle wax

are not d. Because the molecules of liquid candle wax can easily move past one another but the molecules

of solid candle wax cannot

5. You drink all of the water from a plastic bottle. You put the cap on the bottle and tighten it. Then you put the bottle in the refrigerator. An hour later, you notice that the bottle is dented. Why is the bottle dented after being cooled in the refrigerator?

a. All the molecules of air went out of the bottle. b. Heat molecules inside the bottle were destroyed. c. The molecules of air inside the bottle broke down. d. The molecules of air inside the bottle got closer together.

6. A glass thermometer has a colored liquid inside it. The level of colored liquid rises when the thermometer is placed in hot water.  Why does the level of liquid rise?

a. Water molecules are pushed into the thermometer. b. Heat molecules push the molecules of the liquid upward. c. Heat causes the molecules of the liquid to get farther apart. d. The molecules of the liquid break down into atoms and take up more space.

7. How do the molecules of hot air differ from the molecules of cold air? a. The molecules of hot air are farther apart than the molecules of cold air. b. The molecules of hot air have less mass than the molecules of cold air. c. The molecules of hot air have more heat molecules mixed with them. d. The molecules of hot air are smaller than the molecules of cold air.

8. How do the molecules of cold water differ from the molecules of hot water? a. The molecules of cold water are larger than the molecules of hot water. b. The molecules of cold water have fewer heat molecules mixed with them. c. The molecules of cold water have more mass than the molecules of hot water. d. The molecules of cold water are closer together than the molecules of hot water.

Describe how matter is classified by state of matter and by composition1. Which of the following materials cannot be broken down into a simpler form?

a. Compoundb. Solutionc. Mixtured. Element

2. What would the following be classified as: Na. Elementb. Compoundc. Mixtured. Chemical reaction

3. What would the following be classified as: Sia. Elementb. Compoundc. Mixtured. Chemical reaction

4. Which of the following is an element?a. Propaneb. Carbonc. Salt d. Brass

5. Which of the following is an element?a. Steelb. Sodiumc. Butaned. Acetone

6. Which of the following is an element?a. C2H8

b. Gec. NaCl2

d. H + O2 H2O

7. Which of the following is an element?a. Fe2O3

b. Auc. C4H10

d. (CH3)2CO

8. What would the following chemical formula be classified as: CO2

a. Elementb. Compoundc. Mixtured. Chemical reaction

9. What would the following chemical formula be classified as: H2Oa. Elementb. Compound

c. Mixtured. Chemical reaction

10. Which of the following is a compound?a. Propaneb. Carbonc. Chlorined. Ocean water

11. Which of the following is a compound?a. Airb. Sodiumc. Butaned. Oxygen

12. Which of the following is a compound?a. C2H8

b. Gec. Hgd. H + O2 H2O

13. Which of the following is a compound?a. Airb. Auc. Ud. (CH3)2CO

14. What would the following be classified as: Aira. Elementb. Compoundc. Mixtured. Chemical reaction

15. What would the following be classified as: Ocean watera. Elementb. Compoundc. Mixtured. Chemical reaction

16. Which question is most appropriate when trying to identify whether a mixture is homogenous?a. Dos the mixture have a uniform appearance?b. Is the mixture heavy or light?c. Does the mixture contain any bubbles?d. Is the mixture warm or cool?

17. Which question is most appropriate when trying to identify whether a mixture is heterogenous?a. Dos the mixture have a uniform appearance?b. Is the mixture heavy or light?c. Does the mixture contain any bubbles?d. Is the mixture warm or cool?

Explain the difference between chemical and physical changes and demonstrate how these changes can be used to separate mixtures and compounds into their components

1. In which state of matter are the molecules spaced farthest apart? a. A gas b. A liquid c. A solid d. All are equal.

2. In which state of matter are the molecules packed tightly together? a. A gas b. A liquid c. A solid d. All are equal.

3. In which state of matter do the molecules take the shape of their container? a. A gas b. A liquid c. A solid d. All are equal.

4. Use the picture below to explain which phase of matter would have the most energya. solid, left pictureb. liquid, center picturec. gas, right pictured. all 3 have the same energy

5. Use the picture below to explain which phase of matter would have the least energy

a. solid, left pictureb. liquid, center picturec. gas, right pictured. all 3 have the same energy

6. Use the picture below to explain which phase of matter would have the 2nd most energya. solid, left pictureb. liquid, center picturec. gas, right pictured. all 3 have the same energy

7. Ice was placed in a beaker and heated for ten (10) minutes. Data was collected and graphed below. Using the Phase Change graph of water pictured below, where would you find ice and liquid water in the beaker together?

a. Ab. Bc. Cd. D

8. Using the Phase Change graph below, explain what is happening at the location marked A?

a. Liquid is the only thing being heated

b. There is solid and liquid together being heatedc. Liquid is being heated and is turning to the gas phased. There is only the gas phase left being heated

9. Using the Phase Change graph below, explain what is happening at the location marked B?a. Liquid is the only thing being heatedb. There is solid and liquid together being heatedc. Liquid is being heated and is turning to the gas phased. There is only the gas phase left being heated

10. Using the Phase Change graph below, explain what is happening at the location marked C?a. Liquid is the only thing being heatedb. There is solid and liquid together being heatedc. Liquid is being heated and is turning to the gas phased. There is only the gas phase left being heated

11. Using the Phase Change graph below, explain what is happening at the location marked D?a. Liquid is the only thing being heatedb. There is solid and liquid together being heatedc. Liquid is being heated and is turning to the gas phased. There is only the gas phase left being heated

12. Metal at a very high temperature (liquid) is left to cool down over a period of time and is eventually in a solid state. Which phase change of matter BEST describes this scenario?

a. meltingb. freezingc. condensationd. sublimation

13. A piece of dry ice (solid CO2) sitting on a plate turns to gas. Which phase change of matter BEST describes this scenario?

a. meltingb. condensationc. vaporizationd. sublimation

14. A small puddle of water outside disappears after a few days. Which phase change of matter BEST describes this scenario?

a. meltingb. condensationc. vaporizationd. sublimation

15. Water forms on the outside of a window in the morning. Which phase change of matter BEST describes this scenario?

a. freezingb. condensationc. vaporizationd. sublimation

16. A chemical reaction in which energy is absorbed is _____________.a. exothermic

b. endothermicc. both exothermic and endothermicd. none of these are correct

17. Melting a glass bottle into a lump of glass is an example of a ________________. a. physical changeb. chemical changec. industrial changed. all of these are correct

Define chemical and physical properties and compare them by providing examples1. A physical property of zinc metal is _______.

a. Its colorb. Whether or not it burnsc. How it reacts with nitrogen gasd. Whether it changes when placed in an acid

2. A physical property of steel is _______.a. Whether or not it reacts with oxygen to form rustb. How it reacts with Hydrogen gasc. Its shaped. Whether it changes when placed in a base

3. A physical property of Sulfur is _______.a. Whether or not it burnsb. Its ability to react with oxygenc. Its smelld. Its chemical formula

4. Which is a chemical property of copper?a. has a boiling point of 2567° Cb. reacts in air to form a green layerc. has the symbol Cud. is a solid at room temperature

5. Which is a chemical property of Mercury?a. Has a density of 13.6 g/cm-3 at 20o Cb. reacts with Cl to form an insecticidec. has no odord. is a liquid at room temperature

6. Which is a chemical property of gold?a. has a melting point of 1062o Cb. reacts with Chlorine to form Auric chloridec. has the symbol Aud. is a solid at room temperature

AtomsState the three laws that support the existence of atoms

1. Which of the following laws support the existence of atoms?a. Coulomb’s Lawb. Law of multiple proportionsc. Boyle’s Lawd. 2nd Law of thermodynamics

Atomic Theory 1. Dalton suggested that atoms were indestructible and unchangeble to explain:

a. why elements combine in fixed weight ratios to form compounds b. why elements are characterized by the mass of their atoms c. why mass is conserved in chemical reactions d. why compounds combine in fixed weight ratios in chemical reactions

2. Hydrogen combines with oxygen in a 1:8 weight ratio to form water. If every molecule of water contains two atoms of hydrogen and one atom of oxygen, an atom of oxygen must weigh:

a. 8 times the mass of a hydrogen atom b. 1/8 times the mass of a hydrogen atomc. 16 times the mass of a hydrogen atom d. 1/16 times the mass of a hydrogen atom

Describe the contributions of Dalton, Thomson, Rutherford, Bohr and Schrodinger to Atomic structure1. Experiments with cathode rays led to the discovery of the

a. Protonb. Nucleusc. Neutrond. Electron

2. In the gold foil experiment, most of the particles fired at the foila. bounced backb. were absorbed by the foilc. passed through the foild. combined with the foil

3. The gold foil experiment led to the discovery of thea. Electronb. Nucleusc. Cathode rayd. Neutron

4. A nuclear particle that has about the same mass as a proton, but with no electrical charge, is called a(n)a. Nuclideb. Electronc. Neutrond. Isotope

5. The mass of a neutron isa. about the same as that of a protonb. double that of a protonc. about the same as that of an electrond. double that of an electron

6. An aluminum isotope consists of 13 protons, 13 electrons, and 14 neutrons. Its mass number isa. 13b. 14c. 27d. 40

7. Isotopes of an element contain different numbers ofa. Electronsb. Neutronsc. Protonsd. Nuclides

8. The number of protons in one atom of an element is that element’sa. Mass numberb. Atomic numberc. Balanced charged. Isotope

9. Isotopes are atoms of an element with identical a. masses but different abundances. b. masses but different chemical properties. c. chemical properties but different masses. d. abundances but different masses.

10. The weighted average of the masses of stable isotopes of an element as they occur in nature is called the a. average atomic mass. b. atomic weight. c. atomic mass. d. atomic mass unit.

11. The isotope used as a standard for measuring atomic masses is a. carbon-12. b. carbon-14. c. hydrogen-1. d. oxygen-16.

12. The mass of the carbon-12 isotope is a. 12.00 grams. b. 1.00 grams. c. 1.00 atomic mass units. d. 12.00 atomic mass units.

ElectronsBohr Model

1. According to Bohr’s theory, an excited atom woulda. collapse.b. produce line-emission spectra.c. gain energyd. lose energy.

Explain how the color of light emitted by an atom provides information about electron energy levels1. What important conclusion was reached through the study of cathode rays?

a. Cathode rays were proven to be light rays indicating that atoms were indeed indivisible. b. Cathode rays were shown to be positively charged particles indicating that atoms contained

electric charge. c. Cathode rays were shown to be neutral particles with mass. d. The ratio of the charge to mass ratio of particles making up cathode rays was constant, indicating

they were fundamental particles found in all matter.

2. What new concept did Bohr adapt and use to formulate his model of the atom? a. The quantum concept developed by Planck. b. Electromagnetic theory developed by Maxwell. c. Photoelectric theory developed by Thompson. d. Neutron theory developed by Chadwick.

3. What basis did Bohr have for allowing only specific orbits for electrons in his model of the atom? a. Specific orbits were proven experimentally. b. Bohr assumed only specific orbits were allowed. c. Allowed orbits were predicted from electromagnetic theory. d. It was the general consensus of the scientific community.

4. Quantum mechanics considers electron energy levels in an atom and identifies those levels with four quantum numbers. The first, the principal quantum number considers what property of an electron?

a. sublevel b. energy level c. orientation in space d. direction of spin

5. The second, or angular momentum quantum number, considers what property? a. sublevel b. energy level c. orientation in space d. direction of spin

6. The third quantum number, the magnetic quantum number, considers what property? a. sublevel b. energy level c. orientation in space d. direction of spin

7. The fourth quantum number, the spin quantum number, considers what property? a. sublevel b. energy level

c. orientation in space d. direction of spin

8. The distribution of electrons in an atom is specified by the quantum numbers of each electron. What important principle governs the assignment of quantum numbers to electrons in an atom?

a. The Schrodinger inclusion principle states that quantum numbers must be assigned to all available electrons.

b. The Heisenberg uncertainty principle states that the exact position and momentum of an electron cannot be determined at the same time.

c. The Pauli exclusion principle states that no two electrons in an atom can have the same four quantum numbers.

d. None of the above

9. The chemical properties of an element are determined by a. the period to which it belongs. b. number of filled energy levels. c. number of electrons in its outer energy levels. d. the total number of electrons.

Cloud Model

1. Most of the volume of an atom is occupied by thea. nucleus.b. electron cloud.c. nuclides.d. protons.

Write the electron configuration and atomic orbital diagram of an atom1. Which of the following would be the correct orbital diagram for the ground-state electron configuration

of O?

a.

b.

c.

d.

e.

2. This s p d f notation is for what neutral element? 1s22s22p63s23p3

a. Pb. Znc. Nad. Ale. B

3. If electrons in an atom have the lowest possible energies, the electrons are in theira. ground states.b. excited states.c. inert states.d. radiation-emitting states.

2. For an electron in an atom to change from the ground state to an excited state,a. energy must be released.b. energy must be absorbed.c. radiation must be emitted.d. the electron must make a transition from a higher to a lower energy level.

3. The number of orbitals for the d sublevel isa. 1b. 3c. 5d. 7

4. Which is the ground-state electron configuration for Mn?a. [Ar] 4s23d5

b. [Ar] 4s33d3

c. [Ar] 4s13d5

d. [Ar] 4s43d2

5. The following Bohr model diagrams describe the number of electrons in different electron shells. Which of the 4 models is incorrect?

6. Which of the following is indicated by the number of dots in the electron dot notation. The number of electrons

a. in the atom. b. in the outer energy level. c. missing from the outer energy level. d. in the inner energy levels.

Periodic TableDescribe the historical origin of the periodic table

1. The properties of the chemical elements in the periodic table occur in ______________. a. ascending sequence b. descending sequence c. no discernable pattern d. repeating patterns

2. This scientist arranged some elements in triads based on their atomic masses and other properties. a. Dobereiner b. Einstein c. Mendeleev

d. Newlands

3. Mendeleev saw that properties of the elements repeated in an orderly way when he organized them according to ______________.

a. decreasing atomic number b. increasing atomic mass c. increasing atomic size d. increasing volume

4. What group of elements was unknown to Mendeleev when he first organized his periodic table?

a. Group 18, the noble gases b. Group 1, the alkali metals c. Group 2, the alkaline earth metals d. the transition elements

5. The statement that the physical and chemical properties of the elements repeat in a regular pattern when they are arranged in order of increasing atomic number is known as the ______________.

a. Dobereiner's hypothesis b. Group theory c. Mendeleev theory d. periodic law

6. Which pair of elements would you expect to have similar properties?

a. F and Ne b. Li and Fe c. Mg and Ti d. Si and Ge

7. Mendeleev predicted the properties of these two elements, which were unknown at the time. a. boron and arsenic b. carbon and silicon c. gallium and germanium d. silicon and aluminum

8. These two elements are liquids at room temperature and pressure. a. lithium and cesium b. mercury and bromine c. mercury and oxygen d. silver and nitrogen

9. Why was Mendeleev's periodic table widely accepted?

a. He organized the first 14 known elements. b. He predicted the existence and properties of undiscovered elements. c. He was the first to notice a pattern of similar properties among elements. d. His periodic table listed all of the elements in the correct order.

Describe the organization of the modern periodic table1. The 1st period (row) of the periodic table includes a total of _______ elements.

a. 1b. 2c. 7d. 32

2. The 2nd period (row) of the periodic table includes a total of _______ elements. a. 2b. 6c. 8d. 18

3. The 1st group (column) of the periodic table includes _______ elements.a. 1b. 2c. 7d. 32

4. The 2nd group (column) of the periodic table includes _______ elements.a. 2b. 6c. 8d. 18

5. How many valence electrons does chlorine havea. 5b. 6c. 7d. 8

6. What do all of the elements in the 2nd group (column) have in common with one another?a. The same number of protonsb. The same number of orbital shellsc. The same number of valence electronsd. The same number of neutrons

7. What do all of the elements in the 15th group (column) have in common with one another?a. The same number of protonsb. The same number of orbital shellsc. The same number of valence electronsd. The same number of neutrons

8. Which statement correctly describes elements in the same group?a. They have the same number of valence electrons.b. They have electrons in the same outermost energy level.c. They have the same atomic radius.d. They must be in the same state of matter.

9. Horizontal rows of the periodic table are known as _______.a. Groupsb. Familiesc. Periodsd. Columns

10. Columns of the periodic table are known as _______.a. Groups/Familiesb. Periods

c. Similaritiesd. Rows

11. Which of the following elements is a noble gas?a. Xeb. Nc. Nid. Na

12. How many valence electrons does an atom of any halogen have?a. 7b. 4c. 6d. 8

13. Which of the following elements is a non-metal?a. Scb. Csc. Zr d. Br

14. Which of the following elements is a transition metal?a. Aub. Nac. Mgd. F

Describe the periodic trends of atomic size, ionization energy, boiling and melting point, electronegativity, electron affinity, and ionic radius

1. Modern periodic law states that properties of elements repeat in a regular pattern when the elements are arranged in order of increasing _______.

a. Densityb. Atomic massc. Atomic numberd. Periodicity

2. In going from left to right in any given row in the periodic table, the size of atoms generally _______.a. Increasesb. Decreasesc. Stays the samed. Changes randomly

3. Trends in the properties of elements in a group or period can be explained in terms ofa. Binding energyb. Atomic numberc. Electron configurationd. Electron affinity

4. Trends in the periodic table indicate that the element with the greatest ionization energy is in which of the following periods and groups?

a. Period 2, Group 1b. Period 7, Group 2c. Period 1, Group 18

d. Period 6, Group 17

5. Electron affinity tends toa. decrease across a period and decrease down a group.b. increase across a period and increase down a group.c. decrease across a period and increase down a group.d. increase across a period and decrease down a group.

6. Which is the best reason that the atomic radius generally increases with atomic number in each group of elements?

a. The nuclear charge increases.b. The number of neutrons increases.c. The number of energy levels increases.d. A new octet forms.

7. Trends in the periodic table indicate that an element in which of the following periods and groups will have the largest cation (positive ion) radius?

a. Period 7, Group 1b. Period 2, Group 2c. Period 4, Group 2d. Period 1, Group 17

8.

Explain the relationship between families of elements and electron configuration1. An element that has an electron configuration of [Ne]3s23p3 is in Group _____ of the periodic table.

a. 2b. 3c. 6d. 15

2. The outer electron configuration of an alkali metal hasa. 1 electron in the s orbital.b. 1 electron in the p orbital.c. 2 electrons in the s orbital.d. 2 electrons in the p orbital.

3. Which one of the following is the correct electron configuration for a ground-state nitrogen atom?

a.

b.

c.

d.4.

Bonding/StructuresIons and Ionic bonding

1. How does a neutral atom become an "ion"?a. by gaining or losing neutrons

b. by gaining or losing electronsc. by gaining or losing protonsd. by adding electron shells

2. When an atom loses an electron, it:a. Becomes a negative ionb. Becomes a positive ionc. Forms a covalent bondd. Gains protons

3. Which of the following is a property of a covalent compound?a. Low melting pointb. Good conductor of electricity c. Form by transferring electronsd. Form by sharing electrons

4. Ions that are made of more than one atom are called:a. Multi-atomic ionsb. Isotopesc. Moleculesd. Polyatomic ions

5. The electron configuration of a fluoride ion F- is:a. 1s2 2s2 2p5b. the same as a neon atomc. 1s2 2s2 2p6 3s1d. the same as a potassium atom

6. Ionic compounds have:a. A positive chargeb. A negative chargec. No electrical charged. A changing electrical charge

7. The symbol Na+ means:a. That this Sodium ion has gained an electronb. That this Sodium isotope has gained an electronc. That this Sodium ion has 1 valence electrond. That this Sodium ion has lost an electron

8. Compared with ionic compounds, molecular compoundsa. have higher boiling points.b. have lower melting points.c. are brittle.d. are harder.

9. Why does the sodium atom to the right lose its valence electron?a. Sodium has a high electronegativityb. Sodium has a low ionization energyc. Sodium has a large atomic radius

d. Electron shielding increases the attraction of the electron to the nucleus.

Covalent bonding1. The electrons involved in the formation of a covalent bond are

a. transferred from one atom to another.b. valence electrons.c. found only in the s-orbitals.d. in filled orbitals.

2. A covalent bond forms when the attraction between two atoms is balanced by repulsion and the potential energy is

a. at a maximum.b. at a minimum.c. zero.d. equal to the kinetic energy.

3. In a double bond, two atoms share a total of _____ electrons.a. 2b. 3c. 4d. 6

4. A covalent bond forms between a nonmetal and a __________.a. Metal c. nonmetalb. Metalloid d. gas

5. Two atoms have a difference in electronegativity of .2, what kind of bond will they form?a. Polar Covalent c. nonpolar covalentb. Ionic d. hydrogen

6. Which of these combinations is likely to have a polar covalent bond?a. Two atoms of similar sizeb. Two atoms of different sizec. Two atoms with different electronegativitiesd. Two atoms with the same number of electrons

7. The table below shows the electronegativities of four elements. Which of the following bonds is the most polar.

a. Carbon-hydrogenb. Carbon-flourinec. Fluorine-flourined. Hydrogen-oxygen

Metallic bonding1. Atoms of copper and iron

a. generally form stable bonds with transition elements.b. have stable electron configurations.c. tend to form cations.d. tend to form anions.

Chemical Formulas and Chemical Names1. What is the formula for the compound formed by calcium ions, Ca2+, and chloride ions, Cl–?

Element ElectronegativityCarbon 2.6Flourine 4.0

Hydrogen 2.2Oxygen 3.4

a. CaClb. CaCl3

c. Ca2Cld. CaCl2

2. Name the compound Zn3(PO4)2.a. zinc potassium oxideb. zinc phosphatec. trizinc polyoxided. zinc phosphite

3. What is the correct name for the compound FeO?a. Iron Oxideb. Iron(II) Oxidec. Iron (III) Oxided. Iron Oxate

4. What is the proper name for the compound N2S4?a. Nitrogen Sulfideb. dinitrogen quadsulfidec. Nitrogen tetrasulfided. Dinitrogen tetrasulfide

5. What is the formula for the compound Lead(IV) Oxide?a. PbOb. Pb4Oc. PbO2

d. PbO4

6. What is the formula for the compound dihydrogen oxide?a. HO2

b. H20c. HOd. H2O2

7. Carbon reacts with chlorine to form CCL4. What is the name of this compound?a. Carbon Chlorideb. 1-carbon 4-chloridec. Tetracarbon chlorided. Carbon Tetrachloride

8. Aluminum (Al) has three electrons in its outer shell. Oxygen (O) needs two electrons to complete its outer shell. What is the chemical formula for Aluminum Oxide?

a. AlOb. AlO2

c. Al2Od. Al2O3

Lewis Structures of Ionic and Covalent Bonds1. When the octet rule is satisfied, the outermost _____ are filled.

a. d and f orbitalsb. s and d orbitals

c. s and p orbitalsd. d and p orbitals

2. Which of the following molecules has two lone pairs of electrons? (draw a picture)a. CH4b. HClc. H2Od. NH3

3. Which of the following is a polar covalent compound?a. H2Ob. NaClc. CCl4d. BeCl2

4. Which of the following is a nonpolar covalent compound?a. NaClb. CCl4c. AlCl3

d. H2O

5. Carbon tetrachloride, CCl4, was used for cleaning fluid because it dissolves grease. Grease isa. Polarb. Semi-polarc. Nonpolard. non enough information to tell

6. The correct Lewis structure for a fluorine atom in a molecule of F2 showsa. four unshared pairs of electrons.b. two shared pair of electrons.c. an octet of valence electrons.d. 2 octets of valence electrons

7. In the Lewis structure to the right, what do the dots represent?a. Shared Electronsb. unpaired valence electronsc. Unshared valence electronsd. a double bond

8. In the Lewis structure above how many electrons are being shared between the carbon atom and one of the oxygen atoms?

a. 2 electronsb. 4 electronsc. 8 electronsd. 0 electrons

10. Hydrogen trioxide, H2O3, a highly unstable and reactive compound, has been prepared recently in small amounts. Which Lewis electron dot structure is most likely to represent the structure of hydrogen trioxide?

a.

b.

c.

d.

Valence Shell Electron Pair Repulsion 1.According to VSEPR theory, which of the following shapes is possible for a molecule with the molecular formula of CH4?

a. Linearb. trigonal pyramidalc. bentd. tetrahedral

2. According to VSEPR theory, which of the following shapes is possible for a molecule with the molecular formula of H2O?

a. Linearb. trigonal pyramidalc. bentd. tetrahedral

3. According to VSEPR theory, which of the following shapes is possible for a molecule with the molecular formula of NH3?

a. Linearb. trigonal pyramidalc. bentd. tetrahedral

4. According to VSEPR theory, which of the following shapes is possible for a molecule with the molecular formula of F2?

a. Linearb. trigonal pyramidalc. bentd. tetrahedral

Which picture is the correct shape for the following molecules.1. SiH42. H2O

3. BeH24. AsH35. AlCl36. BF37. H2S

Chemical ReactionsDescribe the signs that a chemical reaction has taken place?

1. A student mixes two different liquids together. After mixing the liquids, a solid substance forms that cannot be turned back into the starting liquids. The student claims that a chemical reaction occurred. Why is the student correct?

a. Because a solid substance is always formed during a chemical reactionb. Because a new substance is always formed during a chemical reactionc. Because a chemical reaction always occurs when two substances are mixed togetherd. Because the products of a chemical reaction can never be turned back into the starting substances

2. Which of the following statements about chemical reactions is TRUE?a. All chemical reactions are dangerous.b. Some chemical reactions can be reversed.c. Chemical reactions occur only in a laboratory.d. Chemical reactions require starting with at least two substances.

3. Which of the following statements about chemical reactions is TRUE? a. Chemical reactions produce solids, liquids, or gases. b. Chemical reactions produce solids and gases but not liquids. c. Chemical reactions occur between liquids but not between gases or solids. d. Chemical reactions occur between solids and liquids but not between solids and gases.

4. A student determines the density, solubility, and boiling point of two liquids, Liquid 1 and Liquid 2. Then he stirs the two liquids together and heats them. After stirring and heating the liquids, two different liquids form, Liquid 3 and Liquid 4. Then the student determines the density, solubility, and boiling point of Liquids 3 and 4. He concludes that a chemical reaction occurred. How does the student know that a chemical reaction has occurred? Here are his results:

a. The student knows that a chemical reaction has occurred becauseLiquid 3 has different properties than Liquid 4.

b. The student knows that a chemical reaction has occurred becauseLiquid 1 has different properties than Liquid 2.

c. The student knows that a chemical reaction has occurred becauseLiquids 3 and 4 have different properties than Liquids 1 and 2.

  Density (g/mL)

Soluble in Water

Boiling Point (°C)

 

Before stirring and heating

Liquid 1 0.96 Yes 164

Liquid 2 0.81 Yes 118

 

After stirring and heating

Liquid 3 0.87 Yes 166

Liquid 4 1.00 Yes 100

d. The student knows that a chemical reaction has occurred becausea chemical reaction always occurs when two liquids are mixed together.

5. Which of the following is an example of a chemical reaction? a. A marshmallow turning black when heated over a fire b. A powder dissolving in water to make lemonade c. An ice cube melting into a puddle of water d. Salt crystals being crushed into a powder

6. An insoluble solid produced by a chemical reaction in solution is calleda. a precipitate.b. a molecule.c. a reactant.d. the mass of the product.

Explain how conservation laws form the basis for balancing chemical reactions and know what quantities are conserved in physical, chemical, and nuclear changes

1. The diagram below shows molecules before they react in a chemical reaction. Atoms are represented by circles, and molecules are represented by circles that are connected to each other. The different colored circles represent different kinds of atoms.

a. Because there were 6 atoms before the reaction and 6 atoms after the reaction.

b. Because there were 2 kinds of molecules before the reaction and 2 kinds of molecules after the reaction.

c. Because there were 4 white atoms and 2 gray atoms before the reaction and 4 white atoms and 2 gray atoms after the reaction.

d. Because there were 3 molecules before the reaction and 3 molecules after the reaction.

2. A student adds water and sugar to a jar and seals the jar so that nothing can get in or out. The student then weighs the jar containing the water and sugar. After some sugar dissolves, the student weighs the jar and its contents again. What will happen to the weight of the jar containing the water and sugar after some of the sugar dissolves?

a. The weight will stay the same. b. The weight will increase. c. The weight will decrease. d. The weight will depend on how much sugar dissolves.

a.

3. When heated, oxygen reacts with copper to form copper oxide.

If this reaction occurs in a sealed container, will the mass of the container and everything in it increase, decrease, or stay the same and why?

a. The mass will stay the same because the number of each kind of atom stays the same. b. The mass will decrease because two substances combine to form one substance. c. The mass will increase because a new kind of molecule is formed. d. More information is needed to tell if the mass will change.

4. A student places some baking soda and a jar of lemon juice in a plastic bag and seals the bag. She weighs the bag and everything in it. She shakes the bag so that the lemon juice spills out of the jar and mixes with the baking soda inside the bag. The student observes that bubbles form and the bag expands. If the student weighs the bag and everything in it after the bubbling stops and compares the final weight to the starting weight, what will she find out?

a. The final weight will be greater than the starting weight because new atoms are produced during the experiment.

b. The final weight will be less than the starting weight because some of the atoms are destroyed during the experiment.

c. The final weight will be the same as the starting weight because the number of each kind of atom does not change during the experiment.

d. The final weight will be the same as the starting weight because some atoms are destroyed, but new ones are created during the experiment.

5. A student places a living plant in a jar and seals it so nothing can get in or out. He determines the total mass of the jar and everything inside it. Several weeks later, the plant is dead. What will happen to the total mass of the jar and everything inside it after the plant dies?

a. The mass will stay the same.b. The mass will increase.c. The mass will decrease.d. It depends on the type of plant.

6. In the diagrams below, atoms are represented by circles, and molecules are represented by circles that are connected to each other. The different colored circles represent different kinds of atoms. A propane molecule is made up of 3 carbon atoms and 8 hydrogen atoms. An oxygen molecule is made up of 2 oxygen atoms.

This diagram shows one propane molecule and five oxygen molecules.

Write and balance chemical equations, given the names of reactants and products5. The products of the reaction, C2H5OH + 3O2 2CO2 + 3H2O have the same _____ as the reactants.

a. atoms.b. molecules.c. coefficients.d. subscripts.

6. To balance a chemical equation, it may be necessary to adjust thea. coefficients.b. formulas of the products.c. subscripts.d. number of products.

7. Which of the following is a correctly balanced formula equation CaO + H2O  Ca(OH)2?a. 2CaO +  H2O Ca(OH)2

b. CaO + 2H2O  Ca(OH)2

c. CaO + 2H2O  2Ca(OH)2

d. CaO + H2O  Ca(OH)2

8. Which of the following is a correctly balanced equation for the reaction: __C3H6 + __O2 __ CO2 + __H2O a. 2C3H6 + 9O2 - - > 6CO2 + 3H2O

b. 2C3H6 + 9O2 - - > 6CO2 + 6H2O c. 2C3H6 + 9O2 - - > 3CO2 + 3H2O d. 2C3H6 + 6O2 - - > 6CO2 + 6H2O

9. Which of the following is a correctly balanced equation for the reaction: __K2O __K + __O2a. 2K2O - - > 4K + O2b. 2K2O - - > 2K + 2O2c. K2O - - > K + O2d. 2K2O - - > 5K + O2

10. What is the balanced equation of the reaction: tin(IV) oxide reacts with hydrogen to produce tin and water.a. SnO2 + H2 Sn + H20b. SnO2 + 2H2 Sn + 2H20c. 2SnO2 + 4H2 2Sn + 4H20d. SnO2 + H2 Sn + 2H20

Describe what is represented, on a molecular basis by chemical equations

1. In the diagrams below, sulfur atoms are represented by gray circles, carbon atoms are represented by black circles, and oxygen atoms are represented by white circles. Which of the following could be a product of the chemical reaction between sulfur and oxygen?

b.

c.

d.

e.

4. What is the first step of any chemical reaction?a. Reactants must collide with each otherb. Reactants must collide with each other in the correct orientationc. The reactants must be stirredd. The reactants must be heated

Classify chemical reactions as being synthesis, decomposition, single replacement, or double replacement reactions

1. What type of reaction has the general form AB → A + B. a. ion exchange b. replacement c. decomposition d. combination

2. What type of reaction has the general form AB + C → AC + B. a. ion exchange b. replacement c. decomposition d. combination

3. The reaction Cl2(g) + 2KBr(aq) 2KCl(aq) + Br2(l) is a(n)a. synthesis reaction.b. Single displacement reaction.c. ionic reaction.d. combustion reaction.

4. The reaction 2C2H6 + 7O2 4CO2 + 6H20 is a(n):a. Synthesis reactionb. Single displacement reactionc. Decomposition reactiond. Combustion Reaction

Predict the products of synthesis, combustion, and decomposition reactions and write balanced equations for these reactions

1. Choose the correct statement about combination and decomposition reactions. a. Burning of nonmetals in air leads to a combination reaction. b. Burning of nonmetals in air leads to a decomposition reaction. c. Energy in the form of heat or electric current is released in decomposition reactions. d. Energy in the form of heat or electric current is required for combination reactions.

2. Which is the correct balanced equation for the reaction where the reactants are Na + Cl a. Na(s) + Cl(g) NaCl(s)b. 2Na(s) + Cl(g) 2NaCl(s)c. 1Na(s) + 2Cl(g) NaCl2(s)d. 2Na(s) + 2Cl(g) 2NaCl(s)

3. What is the correct balance equation for the reaction where the reactions are C2H8 + O2 a. 2C2H8 + 8O2 4CO2 + 8H2Ob. C2H8 +4 O2 2CO2 + 4H2Oc. 2C2H8 + 7O2 CO2 + 4H2Od. C2H8 + O2 C2H8O2

Predict products of single replacement reactions, using the activity series, and write balanced equations for these reactions

1. According to the activity series lead can hold its electrons better than chromium. Based on this information choose the incorrect statement.

a. Chromium must be chemically more active than lead. b. Lead must be chemically more active than chromium. c. Chromium will replace any lead ion in solution. d. The energy involved in replacement reactions is usually less than the energy involved in

combination or decomposition reactions.

2. Using the activity series on your formula sheet, determine the correct balanced equation for the reactants KCl + Fe

a. KCl + 2Fe FeCl2 + Kb. KCl + Fe FeCl + Kc. 2KCl + 2Fe KFe + Cl2d. This reaction wouldn’t occur

3. Using the activity series on your formula sheet, determine the correct balanced equation for the reactants PbF2 + Mg

a. PbF2 + Mg PbMg + F2

b. PbF2 + Mg MgF2 + 2Pbc. PbF2 + Mg MgF + Pbd. This reaction wouldn’t occur

Predict products of double replacement reactions, using solubility charts to identify precipitates, and write balanced equations for these reactions

1. Identify the products of the double displacement reaction below: MgF2 + Li2CO3 ???a. Mg(CO3)2 & LiF2

b. CO3F & MgLi2

c. MgCO3 & LiFd. MgCO3 & LiF2

2. Determine the correct balanced equation for the reaction of the reactants: RbNO3 + BeF2 a. RbNO3 + BeF2 BeNO3 + RbF2

b. 2RbNO3 + BeF2 BeNO3 + 2RbFc. 2RbNO3 + BeF2 Be(NO3)2 + 2RbFd. RbNO3 + BeF2 RbBe + FNO3